The heat of combustion of carbon to $C O_{2}$ is $- 393.5 k J / m o l$ . The heat released upon formation of $35.2 g$ of $C O_{2}$ from carbon and oxygen gas is:

- 630 k J

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- 3.15 k J

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- 315 k J

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+ 315 k J

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Solution

The correct option is C $- 315 k J$
Formation of $C O_{2}$ from carbon and dioxygen gas can be represented as

$C (s) + O_{2 (g)} ⟶ C O_{2 (g)}; Δ_{f} H = - 393.5 k J {mol}^{- 1}$

$(1 m o l = 44 g)$

$Heat released on formation of 44 g C O_{2} = - 393.5 k J {mol}^{- 1}$
$Heat released on formation of 35.2 g C O_{2} = \frac{- 393.5 k J {mol}^{- 1}}{44 g} \times 35.2 g = - 315 k J$

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